Cannabis Acetate

Just to reiterate. If you don't have proper licensing and you don't want to have a meeting with the DEA, do not even attempt to purchase acetic anhydride.

This is a chemical which appears high on the top 10 of suspicious chemicals for the DEA, and selling it ANYWHERE in the US requires documentation be sent to the DEA regarding the sale.

This is literally, in the DEA's eyes, a dead giveaway that you intend to produce drugs--usually heroin.


I was sorta hoping you knew something I didn't here Gray--I've been looking for a safe method of obtaining acetic anhydride (through synthesis) and there doesn't seem to be one--they all are very dangerous and use chemicals which should never be mixed with food grade products.

One possible route, for instance, produces phosgene gas. As Gray said, this is very unsafe stuff to be handling improperly. As you graduate up the chemical reagent ladder it becomes much more important what solvent you're using, chemicals you're adding.

Chloroform is indicated for extractions of marijuana--say that someone tried to the acid reflux method for producing the delta-9 variant of THC. Say they decided to use Nitric Acid (which is strong and would likely work for the reaction albeit at reduced efficiency)--Well, that would probably kill them, but it'd be odorless and they wouldn't even know they were dead till a week later when pulmonary edema started to develop.


All that said, I really wish I could have some of the acetate ester--but it's not currently in the cards.

 

Ok, this the answer I was looking for in the other thread. I have a question though. Can you use sulfuric acid as a substitute to acetic anhydride?

 

NO there is no replacement theres only a way to dehydrate a certain liquid maybe white vinigar to make your acetic acid or what ever the hell it is

 

There are definitely no known safe methods for producing acetic annhydride which would be reasonable for use with products intended for ingestion. There is no substitute for acetic annhydride in this reaction--it is a required reagent.

Sulfuric acid *can*, however, be used to isomerize THC under certain conditions (though this will likely destroy/alter many terpenes and other wanted chemicals in the process).

 

crazy thread here.... amazing looking pics

 

That the color becomes a deeper red is not surprising. If you remember the thread way back where we discussed this with jump--I ultimately ended up finding a few various spectral results which suggested that THC in its pure form will appear red.

 

So when people talk about having smoked Cherry Oil.. is that what it is?
Also, is it possible to make Acetic Anhydride by boiling down plain white vinegar for a long ass time?

 

ahh acetetic anhydride!
sometimes you just gotta take the risk squiqqs, ohhh what i could do with a few litres

 

pretty sure thats a negatory...i jean the boiling down vinegar ...good thought tho.! =)
sciencelab.com ...mmm
swim may have ordered acetic off there... i heard when they asked him for an loi, he googled it and wrote one really quick, worked like a charm...no issues..special delivery..chloro n ace...
granted if u try n order a flat of ace they will prob trip hard...but ordering a few mls or few hundred mls, im pretty sure they know you cant make keys of dope with that lil ass bottle...
no doubt they still look at the loi's im sure...prob dont do much more than that unless its over a certain amount...i mean esp if ur loi on file looks tits,,,
again, could be way off base, just what i would assume..
but yea..no issues w that co..
next is ether...=)
still trying to find an actual legit account of chlor extraction...
anyone??

@ gw
sooo if one had all nec equipment n ingredients, is this something i am gonna be able to do, with a decent iq and no real scientific training? lol

also few ?s on the acetate...
have u made it from flowers, and how much better do u think it would be
also do u really gain weight when u do the acetate...? i think ive read that a few places...
so potentially if u tested the acetate it would come back really close to 100%?? or....
just curious what affect this actually has on product...ive made stuff at over 80, but that same stuff, if u took it n did the acetate process on it, would it go up to like 100 or close? or just be a different product but still about as potent?
ill tAKE my answers off the air!
thnx

 

hmmmm thnx..the homie zoer said u were the authority on el acetate-o
no 411 on chlor ex?

 

Went through this in great detail in the previous post I mentioned (between yourself, me, and Jump). I found several independent sources which describe purified (by chromatography) as a deep red oil--this is further backed up by the wavelengths of greatest absorption which are found in THC which are firmly in the green section of the color wheel (corresponding to a "reflected" color of red).

All of the spectrophotometric data I found showed peak absorption in the green wavelengths. We all know the oil upon first extraction is a light yellow resinous oil. When mixing oils like this--the resulting color is not always a function of the color of the individual oils--as these substances (with many double bonds) can conjugate differently when they are in a mixture. This is even more expected when you're dealing with light-active compounds (which THC and most terpenes are).

I believe this is a case of the right hand not always knowing what the left hand is doing as it relates to the science community--this is very common in MJ chemistry, and happens to be one of the main reasons why I've taken up an interest in this field. I find it absolutely deplorable the lack of direction and focus the scientific community has put forth here. The government has scared them all away, it's devious at best--and totally unethical and reprehensible at worst (and in my opinion).

Plainly put, this would normally be one of the first things you'd figure out about a compound--and much of the literature doesn't agree. I focused on papers from the analytical field to get what I felt would be the best answer for this question,these guys tend to have a higher degree of attention to details like this, where a synthetic chemist (which comprise many if not most of the papers on this subject from the chemistry community--excluding biochemistry which is often considered a separate field) may blow over small details like this one. They tend to be more consumed by elucidation of structural nuances and the like.

Look up spectrophotometric data for the stuff and you'll find it agrees with what I've said--the stuff absorbs very strongly in the green wavelengths.

 

I'm really not sure where the post has gotten off to.

As for the anthocyanins, I imagine they play a larger role in an iso/ethanol extraction due to polarity considerations. You're still going to get some of them with a non polar extraction (because of the large ring structures)--but the equilibrium of this extraction is going to depend greatly on the specific anthocyanins at play. These will have very different properties and polarities according to their R groups.

A possible route for removal of these might be either treatment with a strong acid (should destroy many of these), or acidification to a given pH followed by chromatography following a pH as well as a solvent gradient.

A second possibility would be to basify these (strong base) to solubilize them in water preferentially (by creating ions), and then do a liquid-liquid extraction on them. Although I'm unsure what the effects of a strong base might be on our actives--it's possible this might destroy them.

Beyond all of that--these things have crazy amounts of double bonds. That double bonds and their conjugation can play a major role in pigmentation should be more apparent when studying these compounds. Because of conjugation in a ring, when you change one substituent in the ring--you change the electronic properties (energy levels of electrons, etc) throughout the entire ring, usually in a 1:1 shared fashion (if the conjugation is complete).

When double bonds sit close to one another, they are able to share electrons throughout both bonds as if they were one bond (or identical bonds perhaps more correctly). This is never more clear than in benzene. It is for this reason that the conjugated double bonds of benzene can either be drawn as 3 seperate double bonds (which can interconvert)--or as a ring with a circle in the middle (depicting this idea that all of the bonds are equal).

It just also so happens that electrons held in these conjugations have a higher propensity for being active to light found in the visible spectrum (this has mostly to do with energy levels in electron shells, and conjugation between those shells).